Survey
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Study Guide – Honors Chemistry: Final Matter: Different states of matter and key characteristics Mixtures – composition may vary o Heterogeneous o Homogeneous Pure substances o Elements o Compounds – fixed or constant composition Density calculations Chemical vs. physical properties Chemical vs. physical changes Temperature: Celsius to Kelvin and back Roughly boiling and freezing points of water Definition of absolute zero SI unit is Kelvin Experimental definitions: Hypothesis Theory Control Variables Accuracy and precision SI units and simple conversions with standard units, units2, and units 3 Given conversion factors, be able to convert from English to metric units. Sig figs – know how to calculate/determine Rules for significant zeros Rules for calculations o Addition and subtraction o Multiple and division Atoms – Atomic structure o Neutrons o Protons o Electrons Relation to atomic number and weight Dalton’s atomic theory Chapter 2 (2.7 & 2.8), Chapter 7 (7.1, 7.3, 7.5, & 7.6), Chapter 8 (8.1, 8.2, 8.3 & 8.5) Section 2.7: Be able to predict whether an element will form an anion or a cation and what the oxidation state of the ion will be. Predict the ionic charge (oxidation state) of each of the following elements and write the element symbol with the correct format to indicate its charge: Sodium Aluminum Phosphorus Calcium Bromine Selenium Based on ionic charge, be able to predict the ratio with which anions and cations will combine to form a compound. Predict the formula for the following ionic compounds (use your book to remind yourself of some of the polyatomic ions – you will be given a list of names and formulas for polyatomic ions on the exam): Calcium oxide Potassium oxide Aluminum oxide Magnesium chloride Potassium iodide Strontium nitrate Lithium sulfate Nitrogen trihydride Name the following ions: Fe(NO3)2 NH4Cl Ca(Br)2 Al2S3 Chapter 7: How was the original periodic table devised? How is the modern periodic table organized? What is true about elements in the same group? In general, what happens to the size of atoms as measured by atomic radii as you go down a group? Across a period? What happens to the size of ions as you go down a group? Or across a period? How does the size of cations in a period compare to the anions in a period? What is electron affinity and how does it change in general across a period and up or down a group? How does electron affinity compare to electronegativity? What is the most electronegative element in the periodic table? What are some general characteristics of metals? Which are the most metallic element(s) in the periodic table? How does the electron affinity of a metal account for many or all of its properties? What are some general characteristics of nonmetals? How do you explain the metalloids? List the main metalloids. Chapter 8: Be able to distinguish among the three main types of bonds – what is different about each of them?? Ionic – Covalent – Metallic – Be able to draw Lewis dots structures of individual atoms, individual ions, and compounds (both ionic and molecular). Ca and Ca2+ CaCl2 CH4 C2I2 MgO General concepts to review Atomic Structure - history of the development of the modern atomic theory protons neutrons electrons Basic principles of chemical bonding atomic stability in terms of electron configuration nobel gas structures ionic vs. covalent bonding predicting ionic formulas based on ionic charges Periodic trends metals vs. nonmetals atomic size ionic radii electronegativity reactivity similar properties by group Balancing equations - law of conservation of mass Stoichiometry - using balanced equations to determine proportions and yield Limiting reactions - Math concepts to review Metric conversions - including conversions with units squared or cubed - be able to convert given English units to metric Significant figures - rules for determining with addition/subtraction and multiplication/division - purpose of significant figures Balancing chemical equations Moles to grams to moles to number of particles (Avogadro’s number) Stoichiometry with balanced equations Theoretical yield vs. percent yield Limiting reactants